Consider the following half-reaction, for which E° = +1.630 V: HOCl(aq) + H+(aq) + e- ? ½Cl2(g) + H2O(l)
a. Write the acid dissociation reaction for HOCl, including physical states. Although this is not a redox reaction, we can still calculate its potential. [See pages 43-44 of the Equation Guide.] Look up the pKa in Appendix G of Harris, then show that E° = -0.445 V at 25 °C. Repeat for the autoprotolysis of water reaction and calculate its E°.
b. The half-reaction above is written for acidic conditions, with H+ and the protonated form of the weak acid. Convert it to basic conditions (writing it with OH- and the deprotonated form of the weak acid) by combining the half reaction above with the reactions you wrote in part a, then calculate its E°.
c. Calculate E°′ (pH 7) for the original half-reaction.
Please show any needed work.